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Problem: You may want to reference (Pages 145 - 148) Section 4.5 while completing this problem.The commercial production of nitric acid involves the following chemical reactions:4 NH3(g) + 5O2(g) → 4 NO(g) + 6 H2O(g)2 NO(g) + O2(g) → 2 NO2(g)3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)In the following redox reaction identify the element undergoing oxidation and the element undergoing reduction.2 NO(g) + O2(g) → 2 NO2(g)

FREE Expert Solution

To do so, we need to identify the change in oxidation state for each element in the reaction. 

Recall the mnemonic for redox reactions:

Loss Electrons → Oxidation → Reducing Agent

Gain Electrons → Reduction → Oxidizing Agent



Reaction: 2 NO(g) + O2(g) → 2 NO2(g)

Reactants:

For NO: 

This is neither a peroxide nor superoxide, which means O.S. of O = –2.

This is also a neutral compound so the total oxidation state is zero.

O.S. of N + O.S. of O = 0

O.S. of N + (–2) = 0

O.S. of N = +2


For O2

This is an atom in its elemental form, which means O.S. of O = 0.


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Problem Details

You may want to reference (Pages 145 - 148) Section 4.5 while completing this problem.

The commercial production of nitric acid involves the following chemical reactions:

  1. 4 NH3(g) + 5O2(g) → 4 NO(g) + 6 H2O(g)
  2. 2 NO(g) + O2(g) → 2 NO2(g)
  3. 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

In the following redox reaction identify the element undergoing oxidation and the element undergoing reduction.

2 NO(g) + O2(g) → 2 NO2(g)


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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Redox Reactions concept. If you need more Redox Reactions practice, you can also practice Redox Reactions practice problems.